Periodic Table Stuff

IA

The Akali Metals

• Family does not include hydrogen, even though it contains 1 outer electron, which all the other elements of this column do too.

• 100% metallic

• very soft and low density, can be cut by butter knife.

• very reactive with h20 (produce H2 gas - meaning flammable), explosive

• must be stored in kerosene to prevent reaction with air and water

• most reactive group of metals of entire periodic table

• cannot be found in nature on its own, has to be extracted from a compound.

• all lose 1 outer electron to form +1 cation

• reacts readily with members of VIIA (the halogens) to form many salts together, “ionic compounds”

IIA

The Akali(similar to Akali Metals, Akali means not acidic, so basic) Earth (found in the dirt) Metals.

• important to areas that dela with botany, agriculture, norticulture, farming, etc.

  • presence increases pH

  • absences decreases pH( acidic)

• not as reactive as IA, but still found as compounds (must be chemically extracted)

• harder, deeper than IA

• don’t need special storage like IA

• all have two outer electrons that they will lose when they react to form +2 cations

IIIA

The Aluminum Group

• Boron is a nonmetal, remainder of the family is metallic.

• 3 outer electrons (including Boron) lost when they react to form +3 cations.

allotropes

2 or more forms of the same element existing in the same physical state, has vastly different chemical and physical properties due to how the atoms of element are bonded to one another.

IVA/14

The Carbon Group

• contains all 3 element types

• Carbon (non metal) has allotropes (Diamond + Graphite), this will gain 4 electrons to form -4 anions

• Tin and Leads (metals) will lose either 2 or 4 electrons to form +2 or +4 cations.

• Silicon + Germanium can gain or lose electrons.

• Carbon is the only element of the P.T that can self-link extensively.

VA(15)

The Nitrogen Group (The Pnictides - choke/suffocate)

• all 3 classes of elements

• Nitrogen + Phosphorus gain 3 electrons to form -3 anions

• As + Sb gain or lose electrons

• Bismuth will lose 3 or 5 electrons to form +3 or +5 cations

• Phosphorus has allotropes: white, black, red.

VIA(16)

The Oxygen Group (aka the Chalcogens - “ore former”)

• Oxygen and Sulfur will gain two electrons to form -2 anions

• Oxygen is 2nd most reactive element of entire P.T., and has 2 allotropes (O2 + O3 (ozone))

VIIA/17

The Halogens (salt-formers)

• completely non-metallic

• most reactive group of non-metals of entire P.T

• Fluorine most reactive element of the ENTIRE P.T.

• all are diatomic molecular elements

  • F2, yellow gas

  • Cl2, green gas

  • Br2, orange/brown liquid

  • I2, black/blue solid

• So reactive that they react with one another to form inter(between) halogens compounds

• all react with Hydrogen to form hydroholic acids

  • HCl, hydrochloric acid

  • HF, hydrofluoric acid

  • HBr, hydrobromic acid

  • HI, hydoriodic acid

• all gain 1 electron to form -1 anion when they react.

VIIIA/18

The Noble (regal, honorary, high-ranking, aristocratic) Gases

• Prior to 1962, this family was called the Inert (does nothing, completely unreactive) Gases

  • He, Ne, + Ar are 100% Inert, but Kr + Xe react limitedly

• most stable group of elements of entire P.T, filled s orbital and p orbital

• most found in “neon - lights” (red/orange)

Hydrogen

• does not belong to any chemical family

• to be stable: H2 - gas at 25 degrees Celsius

  • non-metallic

  • very flammable

• electron configurate = 1s1

• lose 1 electron when it combines with other non metals: H+, meaning it just has a proton, which is why its called a proton.

• gains 1 electron when it combines with metals + metalloids, H-

• most abundant element of the entire universe

• lightest element of the universe : 2.02g/mol (molar mass)

IB through VIIIB

Transition Metals

• 100% metal

• all solids at 25 degrees Celsius with exception Hg (liquid)

• form a variety of colorful solutions when their compounds are dissolved in water

• all are ductile, malleable, tensile, have luster, and are excellent heat and electricity

• form multiple charges when they form cations (lose electrons)

The Inner Transition Metals

between 5d1 and 5d2, 6d1 and 6d2, make up “f” block

2 series:

• Lanthanides (La), Actinides (Ac) - resemble the first element, difficult to isolate

• Lanthanides make up a lot of high-end electronics, Actinides are mostly radioactive, also called Transuranium Elements

Ions

+4, means lost 4 electrons

-4, means gains 4 electrons

Why do atoms react?

Atoms become ions and react with other atoms to gain greater stability, all are Noble-Gas wannabes.

Isoelectronic

The electronic configuration of an ion becomes the same configuration of a different atom.

Nonmetals becoming ions

Nonmetals always gains enough electrons to completely fill the unfilled orbital and as this happens, it becomes isoelectronic to the noble gas that comes right after them on the periodic table.

Nonmetals can also lose electrons due to their ability to react with one another, metals, and metalloids.

Ions of Transition Metals and Inner Transition Metals

First remove the “s” electrons. After “s” electrons are completely removed, then take additionally electrons from “D” orbital.

Why do some Compounds that contain transition metal ions may import a color when dissolved in water? Why do some not have color.

The color is due to a partially filled “d” orbital (through D1 - D9).

• The absence of color is due to 2 reasons:

  • if there is a ‘d’ orbital, it is fully filled.

  • there is no “d” orbital at all.

What are three transition metals that form consistent, always the same oxidation state(charge) when they chemically combine to form compounds.

Silver: Ag +1 cation

Cadmium: Cd +2 cation

Zinc: Zn +2 cation